Chemical Kineti...

$$A(g)\rightarrow B(g)+C(g)$$

For the $$1^{st}$$ order reaction: $$A_{(g)}\rightarrow 2B_{(g)}+C_{(s)}$$, the value of $$t_{\frac {1}{2}}=24\ mins$$. The reaction is carried out by taking a certain mass of $$A$$ enclosed in a vessel in which it exerts a pressure of $$400\ mm\ Hg$$. The pressure of the reaction mixture after the expiry of $$48\ mins$$ will be:

The rate constant $$(k)$$ of a first-order reaction is $$0.0693\ min^{-1}$$. If we start with $$20\ mol\ L^{-1}$$, then it is reduced to $$2.5\ mol\ L^{-1}$$ in:

In the first order reaction the concentration of reactant decreases from $$1.0\ M$$ to $$0.25\ M$$ in $$20$$ minutes. The value of specific rate is:

Calculate the half-life of the first-order reaction, $$C_2H_4O(g)\rightarrow CH_4(g)+CO(g)$$, if the initial pressure of $$C_2H_4O(g)$$ is 80 mm and the total pressure at the end of 20 minutes is 120 mm.

A reaction that is of the first order with respect to reactant A has a rate constant 6 min$$^{-1}$$. If we start with [A]=0.5 mol L$$^{-1}$$, when would [A] reach the value of 0.05 mol L$$^{-1}$$?

For the first order reaction $$A_{(g)}\rightarrow 2B_{(g)}+C_{(g)}$$, the initial pressure is $$P_A=90 mm$$ Hg, the pressure after 10 minutes is found to be 180 mm Hg. The rate constant of the reaction is:

A certain zero order reaction has $$k=0.025\ M sec^{-1}$$ for the disappearance of A. What will be the concentration of A after 15 seconds if initial concentration is 0.5 M?

In the first order reaction, the concentration of the reactant is reduced to 25% in one hour.The half-life period of the reaction is:

For a 1$$^{st}$$ order reaction (gaseous) (constant V, T) $$a A   \rightarrow (b - 1) B + 1 C$$ (with b > a) the pressure of the system rose by $$50 \left ( \frac{b}{a} - 1 \right )$$% in a time of 10 min. The half life of the reaction is therefore: